This video provides a fast way for you to determine if a molecule is polar or nonpolar. It provides examples so you can quickly distinguish nonpolar molecules from those that are polar.
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Here is a list of molecules that are classified as polar or nonpolar:
N2, O2, Cl2, F2, H2
He, Ne, Ar, Xe
CH4, C2H6, CH2=CH2,
CF4, SBr6, BH3, CO2, PCl5,
H2O, NH3, HF, CH3OH, CH3NH2, CH3COOH
OCS, CH3F, SO2

*** PLEASE WATCH WITH ANNOTATIONS ON! SOME INACCURACIES IN GRAPHICS ARE NOTED AND CORRECTED IN ANNOTATIONS. THANKS! ***
Molecules come in infinite varieties, so in order to help the complicated chemical world make a little more sense, we classify and categorize them. One of the most important of those classifications is whether a molecule is polar or non-polar, which describes a kind of symmetry - not just of the molecule, but of the charge. In this edition of Crash Course Chemistry, Hank comes out for Team Polar, and describes why these molecules are so interesting to him.
You'll learn that molecules need to have both charge asymmetry and geometric asymmetry to be polar, and that charge asymmetry is caused by a difference in electronegativities. You'll also learn how to notate a dipole moment (or charge separation) of a molecule, the physical mechanism behind like dissolves like, and why water is so dang good at fostering life on Earth.
--
Table of Contents
Charge Assymetry & Geometric Asymmetry 01:33
Difference in Electronegatives 01:49
Hank is Team Polar 00:33
Dipole Moment 03:49
Charge Separation of a Molecule 04:12
Like Dissolves Like 04:41
Water is Awesome 05:10
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This chemistry video tutorial provides a basic introduction into bond polarity, electronegativity, and the dipole moment of a bond. It explains how to indicate the polarity of a bond and of a molecule using electronegativity and it discusses how to draw the dipole moment of a bond.
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This organic chemistry video tutorial explains how to identify a bond as an ionic bond, polar covalent bond, or a nonpolar covalent bond. Ionic bonds usually consist of metals and nonmetals where as covalent bonds consists of nonmetals. In a nonpolar covalent bond, electrons are shared equally and the electronegativity difference between the two atoms is 0.4 or less. For polar covalent bonds, the electrons are shared unequally between the two atoms and the electronegativity difference is defined to be 0.5 or more.
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This organic chemistry video tutorial explains how to determine which bond is more polar. It also explains how to rank the bonds from least polar to most polar.
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This video looks at how to determine polarity in a molecule by understanding how the bond polarities, molecule shape, and outside atoms influence polarity using bond polarity vector addition. This includes a flow chart that guides you through the various decisions needed to determine if a molecule is polar or not.
Wikipedia 1/1/2018: In chemistry, polarity is a separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multipole moment.
Polar molecules must contain polar bonds due to a difference in electronegativity between the bonded atoms. A polar molecule with two or more polar bonds must have a geometry which is asymmetric in at least one direction, so that the bond dipoles do not cancel each other.
While the molecules can be described as "polar covalent", "nonpolar covalent", or "ionic", this is often a relative term, with one molecule simply being more polar or more nonpolar than another. However, the following properties are typical of such molecules.
A molecule is composed of one or more chemical bonds between molecular orbitals of different atoms. A molecule may be polar either as a result of polar bonds due to differences in electronegativity as described above, or as a result of an asymmetric arrangement of nonpolar covalent bonds and non-bonding pairs of electrons known as a full molecular orbital.
Polar molecules[edit]
The water molecule is made up of oxygen and hydrogen, with respective electronegativities of 3.44 and 2.20. The dipoles from each of the two bonds (red arrows) add together to make the overall molecule polar.
A polar molecule has a net dipole as a result of the opposing charges (i.e. having partial positive and partial negative charges) from polar bonds arranged asymmetrically. Water (H2O) is an example of a polar molecule since it has a slight positive charge on one side and a slight negative charge on the other. The dipoles do not cancel out resulting in a net dipole. Due to the polar nature of the water molecule itself, polar molecules are generally able to dissolve in water. Other examples include sugars (like sucrose), which have many polar oxygen–hydrogen (−OH) groups and are overall highly polar.
If the bond dipole moments of the molecule do not cancel, the molecule is polar. For example, the water molecule (H2O) contains two polar O−H bonds in a bent (nonlinear) geometry. The bond dipole moments do not cancel, so that the molecule forms a molecular dipole with its negative pole at the oxygen and its positive pole midway between the two hydrogen atoms. In the figure each bond joins the central O atom with a negative charge (red) to an H atom with a positive charge (blue).
The hydrogen fluoride, HF, molecule is polar by virtue of polar covalent bonds – in the covalent bond electrons are displaced toward the more electronegative fluorine atom. Ammonia, NH3, molecule the three N−H bonds have only a slight polarity (toward the more electronegative nitrogen atom). The molecule has two lone electrons in an orbital, that points towards the fourth apex of the approximate tetrahedron, (VSEPR). This orbital is not participating in covalent bonding; it is electron-rich, which results in a powerful dipole across the whole ammonia molecule.
Resonance Lewis structures of the ozone molecule
In ozone (O3) molecules, the two O−O bonds are nonpolar (there is no electronegativity difference between atoms of the same element). However, the distribution of other electrons is uneven – since the central atom has to share electrons with two other atoms, but each of the outer atoms has to share electrons with only one other atom, the central atom is more deprived of electrons than the others (the central atom has a formal charge of +1, while the outer atoms each have a formal charge of −​1⁄2). Since the molecule has a bent geometry, the result is a dipole across the whole ozone molecule.
When comparing a polar and nonpolar molecule with similar molar masses, the polar molecule in general has a higher boiling point, because the dipole–dipole interaction between polar molecules results in stronger intermolecular attractions. One common form of polar interaction is the hydrogen bond, which is also known as the H-bond. For example, water forms H-bonds and has a molar mass M = 18 and a boiling point of +100 °C, compared to nonpolar methane with M = 16 and a boiling point of –161 °C.
Nonpolar molecules[edit]
A molecule may be nonpolar either when there is an equal sharing of electrons between the two atoms of a diatomic molecule or because of the symmetrical arrangement of polar bonds in a more complex molecule.
Not every molecule with polar bonds is a polar molecule. Carbon dioxide (CO2) has two polar C=O bonds, but the geometry of CO2 is linear so that the two bond dipole moments cancel and there is no net molecular dipole moment; the molecule is nonpolar.

NEW & IMPROVED VIDEO LINK - I've improved this video, check it out (http://youtu.be/4SjSKjmO38c). Determining the Type of Bond Based On Electronegativity. Polar, Nonpolar or Ionic Bonds. This is meant to be an introduction to molecular polarity. Higher order polar covalent molecules are not discussed. Clear & Simple Chemistry Explanation.

Learn to determine if a molecule is polar or nonpolar based on the polarity between bonds and the molecular geometry (shape).
We start with the polarity between bonds using the electronegativity (EN) values on the Periodic Table provided. After that we’ll look at how the shape of the molecule, based on VSEPR, allows us to determine if the entire molecule is polar or nonpolar.
In the video you will also learn how to deal with unbonded electron pairs (lone) and how it affects the symmetry and polarity of molecules.
To help you learn and retain knowledge practice problems, with solutions, are provided throughout the video.
Contents:
- Finding is a bond between two atoms is polar or nonpolar.
- Practice.
- Finding is molecules are symmetrical and how this impacts polarity.
- Practice.
- The role of unbonded electron pairs on molecular shape and polarity.
- Practice
- Wrap up on polar and nonpolar molecules.
Get more chemistry help at http://www.thegeoexchange.org/chemistry/bonding
Molecular Shapes done with PhET's free online website:
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Drawing/writing done in InkScape. Screen capture done with Camtasia Studio 4.0. Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo).

This video is Awesome! Understand Bonding Like Never Before. Polar Covalent, Nonpolar Covalent & Ionic Bonds - This video shows how to determine the type of bond that will form based on electronegativity values. The difference in electronegativity values result in the bond being ionic, non polar covalent or polar covalent. Ionic bonds result from the transfer of electrons, polar covalent from the uneven sharing of electrons and non polar covalent bonds from the even sharing of electrons. Tune in for the video on Polar Molecules.

Electronegativity differences in bonding using Pauling scale. Using differences in electronegativity to classify bonds as covalent, polar covalent, or ionic.
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CLEAR & SIMPLE - What is the difference between polar and nonpolar molecules? Check out this video on Molecular Polarity which makes this EASY. Polar and Non Polar Covalent Molecules - This video explains how to determine if a molecule is polar or non polar. I show you how, based on symmetry alone, a molecule can be determined to polar or non polar. Although I show you the shapes of the molecules, it is important for you to be able to classify the shapes according to the VSEPR Theory, so please learn your shapes. The degree of polarity can be determine to a certain extent by the differences in electronegativity, but I don't cover that in this video. Best wishes in learning.

http://purplebonding.com
A polar molecule is a molecule that has poles -- a positive and negative pole to be exact. To determine whether a molecule is polar, you first need to determine if the bonds between the atoms are polar. Next, you use VSEPR, valence shell electron pair repulsion theory, to predict the shape of the molecule. Some shapes will cause the dipoles to cancel out, much as in an even-sided tug-of-war. Some shapes will be asymmetrical, and the dipoles will not cancel out. These factors explain why carbon dioxide CO2 is nonpolar, whereas water H2O is.
Watch the video to learn more about determining molecular polarity.

ilmkidunya.com has brought to you Lecture of Sibghat Ullah on "9th Class Chemistry Chapter 4 Structure of Molecules.
Topic 4.3.4 Polar & Non Polar Covalent Bond".
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Chemistry: What is a Covalent Bond? (Polar and Nonpolar)
Covalent bonds are one of the 3 main types of intramolecular forces, along with ionic bonds and metallic bonds. Covalent bonds are the result of atoms sharing their valence electrons. Covalent bonds can be polar or nonpolar, depending on the electronegativies of the atoms involved in the bond.
We show five examples of covalent bonds using Lewis dot structure notation: HF, CO2, H2, H2O and CCl4.
You can click on the links below to jump to sections in the lesson:
0:28 Definition of a Covalent Bond
0:42 Example 1: HF (single covalent bond)
1:23 Example 2: CO2 (double covalent bond)
2:09 Nonpolar covalent bonds
2:20 Example 3: H2
2:43 Polar covalent bonds
2:48 Example 4: H2O
3:58 Example 5: CCl4
4:39 Pauling Bond Polarity Scale (Linus Pauling)
5:15 Do covalent bonds break apart in water? (electrolytes)
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This is a video on how you use the differences in the electronegativity of the elements to identify a bond between two elements as polar covalent, nonpolar covalent or ionic. There is also a brief introduction to identifying polar molecules.

https://www.thechemistrysolution.com
This chemistry tutorial covers bond polarity and electronegativity, and the general trend of electronegativity on the periodic table. This tutorial also includes examples determining the relative polarity of different bonds.

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This chemistry video tutorial provides a basic introduction into the types of chemical bonds such as polar covalent bonds, nonpolar covalent bonds and ionic bonds. It discusses the difference between ionic bonding and covalent bonding. Ionic bonds can be identified by looking for a metal combined with a nonmetal. Covalent bonds typically occur among 2 or more nonmetals. Covalent bonding involves a sharing of electrons and ionic bonding forms as a result of a transfer of electrons from the metal to the nonmetal producing ions with opposite charge which are attracted to each other. The electrostatic force of attraction produces the ionic bond that holds the cations and anions together. Polar covalent bonds have unequal sharing of electrons between the atoms where as nonpolar covalent bonding have a relatively equal sharing of electrons between the atoms attached to the bond. Polar covalent bonds typically have an electronegativity difference of 0.5 or more where as nonpolar covalent bonds have a value difference of 0.4 or less. This video contains plenty of examples and practice problems.
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How can you tell the difference between compounds that are ionic and molecular (also known as covalent)? It has to do with the elements that make them up: ionic compounds are made of metals and nonmetals, and molecular (or covalent) compounds are made of nonmetals. We'll learn how they bond differently: in covalent compounds, the atoms share electrons, and in ion compounds, atoms steal electrons and then opposite charges attract. Ionic and molecular (covalent) compounds also look different at the microscopic level: covalent and molecular compounds exist in molecules, while ionic compounds are organized in lattice structures.

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This is an introduction to the basics of VSEPR Theory. VSEPR theory is a set of rules for how to look at a Lewis structure and determine the three dimensional (3D) shape of a molecule. The shapes have to do with the location of bonds and lone electrons pairs. In this video, we'll look at the following shapes: linear, trigonal planar, bent, tetrahedral, and trigonal bipyramidal

In this live tutoring session I focused on electron geometry, molecular geometry & polarity. Enjoy!
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The Tron Roadmap.
Follow us on Twitter , Facebook , Steemit , and join our Telegram channel for the latest blockchain and cryptocurrency news.
With an already existing user base of over 180 million, the opportunities for this Blockchain and cryptocurrency seem enormous. Also, it will likely not have to bootstrap and this is a deviation from the trajectory of most apps and platforms of this nature.
An outsider continues to steal the crypto spotlight.
Investors started telling CoinDesk in late December that Telegram was looking at doing some kind of ICO.
All that on top of promising super fast payments and micropayments using mobile devices, with negligible transaction fees.
With these announcements, fake sites quickly popped up claiming to be the place to buy grams. Confirming that one was fake in a tweet proved to be the closest Durov has come to a public confirmation of the crowdsale.

By mid-month, the idea that Telegram might raise its fundraising round even higher was reported by Bloomberg.
Early February.
They come up with a lockup period that releases tokens after four waiting periods, the longest one last 18 months.
Late February.
Finally, Telegram has apparently offered investors some kind of refund provision if it fails to deliver the TON platform by the end of October 2019, Business Insider reported.
The leader in blockchain news, CoinDesk is a media outlet that strives for the highest journalistic standards and abides by a strict set of editorial policies. CoinDesk is an independent operating subsidiary of Digital Currency Group, which invests in cryptocurrencies and blockchain startups.
The filing names Ton Issuer Inc. and Telegram Group Inc. along with the two individuals, Pavel Durov and Nikolai Durov, as related persons.
Apart from building on the extensive userbase Telegram has amassed, and serving as a medium of exchange with a native cryptocurrency called GRAM, the TON platform also aims to include smart contracts and decentralized services such as TON Storage and TON Proxy.
Leverage and Margin Explained.